Question

Ice Station Bravo near the North Pole launched a helium-filled balloon. What is the volume of the balloon at an altitude of 18,000m where the atmospheric pressure is 0.072atm?

a) 0.0496 m^3
b) 0.496 m^3
c) 4.96 m^3
d) 49.6 m^3

Answer 1

The volume of the balloon at an altitude of 18,000m where the atmospheric pressure is 0.072atm is 13.89 m^3.

Step-by-step explanation:

To calculate the volume of the balloon at an altitude of 18,000m where the atmospheric pressure is 0.072atm, we can use Boyle's Law. Boyle's Law states that the product of pressure and volume is constant, as long as the temperature remains constant. We can set up the following equation:

P1*V1 = P2*V2

Where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume. Rearranging the equation, we can solve for V2:

V2 = (P1*V1) / P2

Plugging in the given values:

V2 = (1 atm * V1) / 0.072 atm

V2 = 13.89 * V1

Since the final volume is 20 times the original volume, we can substitute V1 with 1 and solve for V2:

V2 = 13.89 * 1

V2 = 13.89 m^3